{"id":12719,"date":"2026-06-09T11:13:36","date_gmt":"2026-06-09T11:13:36","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=12719"},"modified":"2026-06-09T11:25:09","modified_gmt":"2026-06-09T11:25:09","slug":"structure-and-properties-of-water-2","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/iit-jam\/structure-and-properties-of-water-2\/","title":{"rendered":"Structure and properties of Water: Master IIT JAM 2027"},"content":{"rendered":"<p><strong>Structure and properties of Water<\/strong> For IIT JAM is a fundamental concept in physical chemistry that deals with the molecular structure, intermolecular forces, and physical properties of water.<\/p>\n<h2><strong>Syllabus: Physical Chemistry for IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"4\">If you look at the official <a href=\"https:\/\/jam2026.iitb.ac.in\/files\/syllabus_BT.pdf\" rel=\"nofollow noopener\" target=\"_blank\"><strong>IIT JAM syllabus<\/strong><\/a>, the <b data-path-to-node=\"4\" data-index-in-node=\"51\">Structure and properties of water sit<\/b> comfortably inside Unit 1 under atomic and molecular structure. For IIT JAM and CUET PG, it ties directly into chemical bonding, intermolecular forces, and thermodynamics.<\/p>\n<p data-path-to-node=\"5\">Standard reference books like <i data-path-to-node=\"5\" data-index-in-node=\"30\">Atkins&#8217; Physical Chemistry<\/i> or McQuarrie &amp; Simon&#8217;s <i data-path-to-node=\"5\" data-index-in-node=\"80\">Physical Chemistry: A Molecular Approach<\/i> dive deep into this. Since IIT JAM uses a mix of Multiple Choice Questions (MCQs), Multiple Select Questions (MSQs), and Numerical Answer Type (NAT) questions\u2014complete with negative marking for Section A\u2014you need to know the &#8220;why&#8221; behind water&#8217;s behavior, not just memorize facts.<\/p>\n<h2><strong>Molecular Structure of Water: A Key Aspect of Structure and properties of Water For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"8\">Let&#8217;s look at a single molecule of H\u2082O.\u00a0You already know it has a bent, or V-shape, geometry. But let&#8217;s look at why.<\/p>\n<p data-path-to-node=\"9\">As per <strong>Structure and properties of Water, <\/strong>the oxygen atom undergoes <span class=\"math-inline\" data-math=\"sp^3\" data-index-in-node=\"26\">sp3<\/span> hybridization. In a perfect tetrahedral world, the bond angle would be <span class=\"math-inline\" data-math=\"109.5^\\circ\" data-index-in-node=\"102\">109.5\u00b0<\/span>. However, oxygen brings two lone pairs to the party. According to VSEPR theory, those lone pairs take up a lot of space and push the two O-H bonding pairs closer together, squeezing the bond angle down to about <span class=\"math-inline\" data-math=\"104.5^\\circ\" data-index-in-node=\"325\">104.5\u00b0<\/span>.<\/p>\n<p data-path-to-node=\"10\">Because oxygen is way more electronegative than hydrogen, it pulls the shared electrons closer to itself. This creates a partial negative charge (\u00f0<sup><span class=\"math-inline\" data-math=\"\\delta^-\" data-index-in-node=\"146\">&#8211;<\/span><\/sup>) on the oxygen and a partial positive charge (\u00f0<sup><span class=\"math-inline\" data-math=\"\\delta^+\" data-index-in-node=\"201\">+<\/span><\/sup>) on the hydrogens. Since the molecule is bent, these individual bond dipoles don&#8217;t cancel out. Instead, they add up to give water a strong, permanent electric dipole moment. This high polarity is the secret sauce behind almost all the unique physical and chemical traits we study in the <b data-path-to-node=\"10\" data-index-in-node=\"497\">Structure and properties of Water<\/b>.<\/p>\n<h2><strong>Intermolecular Forces in Water: A Critical Aspect of Structure and properties of Water For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"13\">Moving from a single molecule to a glass of water, how do these molecules talk to each other? The structural quirks we just talked about lead directly to three types of intermolecular forces: <b data-path-to-node=\"13\" data-index-in-node=\"192\">hydrogen bonding<\/b>, <b data-path-to-node=\"13\" data-index-in-node=\"210\">dipole-dipole interactions<\/b>, and <b data-path-to-node=\"13\" data-index-in-node=\"242\">London dispersion forces<\/b>.<\/p>\n<p data-path-to-node=\"14\">The star of the show here is hydrogen bonding. Because water is so polar, the \u00f0<sup><span class=\"math-inline\" data-math=\"\\delta^+\" data-index-in-node=\"78\">+<\/span><\/sup> hydrogen of one water molecule is strongly attracted to the \u00f0<sup><span class=\"math-inline\" data-math=\"\\delta^-\" data-index-in-node=\"147\">&#8211;<\/span><\/sup>\u00a0lone pair of a neighboring oxygen.<\/p>\n<ul data-path-to-node=\"15\">\n<li>\n<p data-path-to-node=\"15,0,0\"><b data-path-to-node=\"15,0,0\" data-index-in-node=\"0\">Hydrogen Bonds:<\/b> These are remarkably strong for intermolecular forces, packing an energy of about 10 to 30 kJ\/mol, and they can operate over distances up to 0.3 nm.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"15,1,0\"><b data-path-to-node=\"15,1,0\" data-index-in-node=\"0\">Dipole-Dipole &amp; London Dispersion Forces:<\/b> Dispersion forces are the weakest link here, sitting at around 0.1 to 10 kJ\/mol with a much shorter range.<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"16\">As per <strong>Structure and properties of Water, <\/strong>this extensive network of hydrogen bonds means water molecules stick together tightly, explaining why it takes so much effort to boil it compared to other similar-sized molecules like H\u2082S.<\/p>\n<h2><strong>Physical Properties of Water: A Practical Application of Structure and properties of Water For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"19\">Now, let&#8217;s see how these microscopic forces show up in the real world.<\/p>\n<p data-path-to-node=\"20\"><strong>The 4\u00b0C Quirk (Anomalous Expansion)<\/strong><\/p>\n<p data-path-to-node=\"21\">Most liquids shrink and get denser as they freeze. Water plays by its own rules. As you cool liquid water, it contracts and gets denser\u2014but only until it hits 4\u00b0C. Below 4\u00b0C, it starts expanding and becoming <i data-path-to-node=\"21\" data-index-in-node=\"208\">less<\/i> dense. When it finally freezes into ice, the molecules lock into a rigid, open, hexagonal crystalline structure held apart by fixed hydrogen bonds.<\/p>\n<p data-path-to-node=\"22\">Imagine a fictional scenario where a lake in northern India freezes over in January. If water behaved like normal liquids, the ice would sink to the bottom, eventually freezing the whole lake solid and destroying the aquatic ecosystem. Because of this anomalous expansion, the ice floats on top. It creates an insulating blanket that keeps the liquid water underneath at a livable 4\u00b0C, keeping the fish happy and alive.<\/p>\n<p data-path-to-node=\"23\"><strong>Thermal Buffer (High Specific Heat Capacity)<\/strong><\/p>\n<p data-path-to-node=\"24\">Water has a massive specific heat capacity\u2014about 4.18 J\/g\u00b0C. Heat capacity is just the amount of heat energy needed to raise the temperature of a substance by 1\u00b0C. Because water has that stubborn network of hydrogen bonds, it can absorb a ton of heat energy before those bonds break and the molecules start moving faster. This is why coastal cities have moderate weather compared to scorching deserts; the ocean acts like a giant, planet-wide thermostat.<\/p>\n<h2><strong>Worked Example: Calculating the Entropy Change of Water<\/strong><\/h2>\n<p data-path-to-node=\"27\">In the IIT JAM physical chemistry section, you are bound to face thermodynamics problems dealing with entropy change (\u0394<span class=\"math-inline\" data-math=\"\\Delta S\" data-index-in-node=\"118\">S<\/span>), which measures the change in system disorder.<\/p>\n<p data-path-to-node=\"28\">Let&#8217;s look at a straightforward problem to see how\u00a0 <strong>Structure and properties of Water<\/strong> works.<\/p>\n<p data-path-to-node=\"28\"><b data-path-to-node=\"29,0\" data-index-in-node=\"0\">Question:<\/b> Imagine you have 1 mole of liquid water at 100\u00b0C (373.15 K) turning into steam at the same temperature. The heat of vaporization (<span class=\"math-inline\" data-math=\"\\Delta H_{vap}\" data-index-in-node=\"140\">H<sub>vap<\/sub><\/span>) for water is <span class=\"math-inline\" data-math=\"40.7 \\text{ kJ\/mol}\" data-index-in-node=\"169\">40.7 kJ\/mol.<\/span>\u00a0Calculate the entropy change (\u0394<span class=\"math-inline\" data-math=\"\\Delta S\" data-index-in-node=\"220\">S<\/span>) for this vaporization.<\/p>\n<p data-path-to-node=\"30\"><b data-path-to-node=\"30\" data-index-in-node=\"0\">Solution:<\/b><\/p>\n<p data-path-to-node=\"30\">Since this phase change happens at a constant temperature, we can use the straightforward entropy formula:<\/p>\n<p data-path-to-node=\"30\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-21879 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/phase-change-happens.png\" alt=\"phase change happens\" width=\"186\" height=\"107\" \/><\/p>\n<p data-path-to-node=\"30\">Here, <span class=\"math-inline\" data-math=\"Q_{rev}\" data-index-in-node=\"6\">Q<sub>rev<\/sub><\/span> is equal to the enthalpy of vaporization (\u0394<span class=\"math-inline\" data-math=\"\\Delta H_{vap}\" data-index-in-node=\"56\">H<sub>vap<\/sub><\/span>). Let&#8217;s convert kilojoules to joules so our units match standard thermodynamic values:<\/p>\n<div class=\"math-block\" style=\"text-align: center;\" data-math=\"Q_{rev} = 40.7 \\text{ kJ\/mol} = 40700 \\text{ J\/mol}\">Q<sub>rev<\/sub>= 40.7\u00a0 kJ\/mol = 40700\u00a0 J\/mol<\/div>\n<div data-math=\"Q_{rev} = 40.7 \\text{ kJ\/mol} = 40700 \\text{ J\/mol}\">Now, divide by the absolute temperature in Kelvin:<\/div>\n<div data-math=\"Q_{rev} = 40.7 \\text{ kJ\/mol} = 40700 \\text{ J\/mol}\"><img loading=\"lazy\" fetchpriority=\"high\" decoding=\"async\" class=\"alignnone size-medium wp-image-21880 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/absolute-temperature-300x202.png\" alt=\"absolute temperature\" width=\"300\" height=\"202\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/absolute-temperature-300x202.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/absolute-temperature.png 332w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/div>\n<div data-math=\"Q_{rev} = 40.7 \\text{ kJ\/mol} = 40700 \\text{ J\/mol}\">The positive value makes perfect sense because gas molecules are way more disordered than liquid molecules.<\/div>\n<h2><strong>Common Misconceptions<\/strong><\/h2>\n<p data-path-to-node=\"40\">When clearing doubts here at <a href=\"https:\/\/www.vedprep.com\/online-courses\/iit-jam\"><b data-path-to-node=\"40\" data-index-in-node=\"29\">VedPrep<\/b><\/a>, we often see students fall into a classic trap: confusing molecular symmetry with bond polarity while dealing with <strong>Structure and properties of Water<\/strong>.<\/p>\n<p data-path-to-node=\"41\">Some students think that because a water molecule seems simple and balanced on paper, the dipoles must cancel out, making it non-polar. Don&#8217;t fall for this! Carbon dioxide (CO\u2082)\u00a0is linear, so its dipoles cancel out to zero. Water is distinctly bent. That asymmetrical V-shape ensures the dipoles reinforce each other, making it highly polar.<\/p>\n<h2 data-path-to-node=\"47\"><strong>Laboratory &amp; Real-World Applications<\/strong><\/h2>\n<p data-path-to-node=\"48\">We see the practical magic of the <b data-path-to-node=\"48\" data-index-in-node=\"34\">Structure and properties of Water<\/b> everywhere. In the lab, its high polarity makes it the &#8220;universal solvent,&#8221; capable of dissolving ionic salts by forming hydration shells around ions.<\/p>\n<p data-path-to-node=\"49\">In environmental science, that ice-insulation phenomenon we discussed earlier is the entire reason aquatic life survives harsh winters. Without the unique crystalline structure of ice and the resulting density drop, life on Earth would look completely different.<\/p>\n<h2 data-path-to-node=\"49\"><strong>Final Thoughts\u00a0<\/strong><\/h2>\n<p data-path-to-node=\"49\">When you sit down to tackle the physical chemistry section of the IIT JAM, remember that the examiners aren&#8217;t just looking for your ability to memorize equations\u2014they want to see if you can connect microscopic structures to macroscopic behavior. The <b data-path-to-node=\"0\" data-index-in-node=\"250\">Structure and properties of Water<\/b> is the perfect sandbox for this. It bridges the gap between quantum mechanical hybridization, thermodynamic energy changes, and real-world environmental phenomena.<\/p>\n<p data-path-to-node=\"49\">To know more in detail from our expert faculty, watch our YouTube video:<\/p>\n<p class=\"responsive-video-wrap clr\"><iframe title=\"Plant Physiology Photosynthesis | Plant Water Relation |CUET PG|JAM| NET| VedPrep Biology Academy\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/r-QVcHAIie8?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe><\/p>\n<section>\n<h2><strong>Frequently Asked Questions<\/strong><\/h2>\n<\/section>\n<style>#sp-ea-21883 .spcollapsing { height: 0; overflow: hidden; transition-property: height;transition-duration: 300ms;}#sp-ea-21883.sp-easy-accordion>.sp-ea-single {margin-bottom: 10px; border: 1px solid #e2e2e2; }#sp-ea-21883.sp-easy-accordion>.sp-ea-single>.ea-header a {color: #444;}#sp-ea-21883.sp-easy-accordion>.sp-ea-single>.sp-collapse>.ea-body {background: #fff; color: #444;}#sp-ea-21883.sp-easy-accordion>.sp-ea-single {background: #eee;}#sp-ea-21883.sp-easy-accordion>.sp-ea-single>.ea-header a .ea-expand-icon { float: left; color: #444;font-size: 16px;}<\/style><div id=\"sp_easy_accordion-1781003222\">\n<div id=\"sp-ea-21883\" class=\"sp-ea-one sp-easy-accordion\" data-ea-active=\"ea-click\" data-ea-mode=\"vertical\" data-preloader=\"\" data-scroll-active-item=\"\" data-offset-to-scroll=\"0\">\n\n<!-- Start accordion card div. -->\n<div class=\"ea-card ea-expand sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218830\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218830\" aria-controls=\"collapse218830\" href=\"#\"  aria-expanded=\"true\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-minus\"><\/i> Why does water have a bent shape instead of a linear one?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse collapsed show\" id=\"collapse218830\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218830\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>The oxygen atom in water goes through <span class=\"math-inline\" data-math=\"sp^3\" data-index-in-node=\"38\">sp3<\/span>\u00a0hybridization, which sets up a tetrahedral arrangement for its electron pairs. Since oxygen has two bonding pairs and two lone pairs, the lone pairs push down on the bonds (thanks to VSEPR theory). This distorts the perfect tetrahedron into a bent, or V-shape.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218831\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218831\" aria-controls=\"collapse218831\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the exact bond angle in a water molecule, and why?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218831\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218831\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>The bond angle is about <span class=\"math-inline\" data-math=\"104.5^\\circ\" data-index-in-node=\"24\">104.5\u00b0<\/span>. In a perfect tetrahedral shape, it would be <span class=\"math-inline\" data-math=\"109.5^\\circ\" data-index-in-node=\"81\">109.5\u00b0<\/span>. However, the two lone pairs on the oxygen atom take up more space and repel the O-H bonding pairs more strongly, squeezing the angle down by about <span class=\"math-inline\" data-math=\"5^\\circ\" data-index-in-node=\"241\">5\u00b0<\/span>.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218832\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218832\" aria-controls=\"collapse218832\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does the polarity of water arise?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218832\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218832\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Polarity comes down to a tug-of-war for electrons. Oxygen is much more electronegative than hydrogen, so it pulls the shared electrons closer to itself. This creates a partial negative charge on the oxygen and a partial positive charge on the hydrogens. Because the molecule is bent, these charges don't cancel out, leaving water with a permanent dipole moment.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218833\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218833\" aria-controls=\"collapse218833\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What type of hybridization does the oxygen atom in water undergo?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218833\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218833\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>The oxygen atom is <span class=\"math-inline\" data-math=\"sp^3\" data-index-in-node=\"19\">sp<sup>3<\/sup><\/span>\u00a0hybridized. It uses four hybrid orbitals: two to form <span class=\"math-inline\" data-math=\"\\sigma\" data-index-in-node=\"78\">$\\sigma$<\/span> (sigma) bonds with the hydrogen atoms and two to hold its lone pairs of electrons.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218834\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218834\" aria-controls=\"collapse218834\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is the hydrogen bond in water stronger than a typical dipole-dipole interaction?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218834\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218834\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Hydrogen bonding is a supercharged version of a dipole-dipole interaction. Because hydrogen is small and bonded to a highly electronegative oxygen, the positive charge density on the hydrogen is incredibly high. This allows it to get very close to the lone pairs of a neighboring oxygen, creating a remarkably strong attraction.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218835\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218835\" aria-controls=\"collapse218835\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What are the typical energy values for hydrogen bonds vs. London dispersion forces in water?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218835\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218835\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Hydrogen bonds in water are relatively strong, packing an energy of about 10 to 30 kJ\/mol. On the flip side, London dispersion forces are much weaker, usually sitting between 0.1 and 10 kJ\/mol.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218836\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218836\" aria-controls=\"collapse218836\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What does the \"anomalous expansion of water\" actually mean?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218836\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218836\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Normally, liquids contract and get denser as they cool down. Water does this too, but only until it hits 4\u00b0C. Below 4\u00b0C, it reverses course and starts expanding, meaning it becomes less dense as it gets colder and freezes into ice.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218837\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218837\" aria-controls=\"collapse218837\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why does ice float on liquid water?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218837\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218837\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>When water freezes, the molecules slow down enough for hydrogen bonds to lock them into a rigid, open, hexagonal crystal lattice. This structure leaves a lot of empty space between the molecules. Because the same mass of water takes up more space as ice, ice ends up less dense than liquid water and floats.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218838\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218838\" aria-controls=\"collapse218838\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why does water have such a high specific heat capacity?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218838\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218838\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It all comes down to that stubborn network of hydrogen bonds. Before water molecules can start moving faster (which raises the temperature), a lot of heat energy has to be consumed just to break those hydrogen bonds. At <b data-path-to-node=\"22\" data-index-in-node=\"220\">VedPrep<\/b>, we like to think of water as a thermal sponge for this exact reason.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-218839\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse218839\" aria-controls=\"collapse218839\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can water form hydrogen bonds with other types of molecules?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse218839\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-218839\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes! Water can form hydrogen bonds with any molecule that has a hydrogen atom bonded to a highly electronegative element (like Nitrogen, Oxygen, or Fluorine) or with molecules that have lone pairs on those same electronegative atoms, like alcohol or ammonia.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2188310\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2188310\" aria-controls=\"collapse2188310\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What type of questions does IIT JAM ask from the Structure and properties of Water?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2188310\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-2188310\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>IIT JAM tests this topic through various formats. You might see MSQs (Multiple Select Questions) asking which statements about water's properties are correct, MCQs on hybridization and bond angles, or NAT (Numerical Answer Type) problems calculating entropy or enthalpy changes during phase transitions.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2188311\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2188311\" aria-controls=\"collapse2188311\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is water called the \"universal solvent\"?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2188311\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-2188311\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Because of its high polarity and large dielectric constant, water is incredibly good at dissolving ionic compounds and polar covalent molecules. It surrounds the solute ions, forming hydration shells that separate and stabilize them in the solution.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2188312\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2188312\" aria-controls=\"collapse2188312\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does water's high specific heat capacity affect Earth's climate?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2188312\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-2188312\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Since oceans can absorb massive amounts of solar heat during the day without a huge jump in temperature, and slowly release that heat at night, they act as a massive global thermostat. This keeps coastal areas from experiencing extreme temperature swings.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2188313\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2188313\" aria-controls=\"collapse2188313\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the difference between a lone pair and a bonding pair in a water molecule?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2188313\" data-parent=\"#sp-ea-21883\" role=\"region\" aria-labelledby=\"ea-header-2188313\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Bonding pairs are the electrons shared between the oxygen and hydrogen atoms to form covalent bonds. Lone pairs are the two sets of valence electrons on the oxygen atom that aren't shared with any other atom but still influence the molecule's overall shape.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<\/div>\n<\/div>\n\n","protected":false},"excerpt":{"rendered":"<p>Understanding Structure and properties of Water For IIT JAM is crucial for students preparing for CSIR NET, IIT JAM, and other competitive exams. This topic deals with the molecular structure, intermolecular forces, and physical properties of water.<\/p>\n","protected":false},"author":11,"featured_media":12718,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","rank_math_seo_score":88},"categories":[23],"tags":[7689,7717,7718,7719,7720,2922],"class_list":["post-12719","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-iit-jam","tag-biology","tag-structure-and-properties-of-water-for-iit-jam","tag-structure-and-properties-of-water-for-iit-jam-notes","tag-structure-and-properties-of-water-for-iit-jam-questions","tag-structure-and-properties-of-water-for-iit-jam-study-material","tag-vedprep","entry","has-media"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12719","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/users\/11"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=12719"}],"version-history":[{"count":5,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12719\/revisions"}],"predecessor-version":[{"id":21885,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12719\/revisions\/21885"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/12718"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=12719"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=12719"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=12719"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}